Electron configuration
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![Page 1: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/1.jpg)
ELECTRON CONFIGURATION Periodic Table
![Page 2: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/2.jpg)
s, p, d, and f ORBITALS
![Page 3: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/3.jpg)
S- Orbital
![Page 4: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/4.jpg)
P - orbitals
![Page 5: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/5.jpg)
D- orbitals
![Page 6: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/6.jpg)
F-orbitals
![Page 7: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/7.jpg)
QUANTUM NUMBERS
![Page 8: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/8.jpg)
• Principal Quantum Number, n
• Azimuthal Quantum Number, l
• Magnetic Quantum Number, ml
![Page 9: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/9.jpg)
Exercise
• What are the similarities and differences between the hydrogen atom 1s and 2s orbitals?
• For n=4 what are the possible values of l and m?
• give the values for n, l, m fora. 2pb. 5dc. 5f
![Page 10: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/10.jpg)
Main Energy Level
No. of Sublevel
Identity of
Sublevels
No. of Orbitals
(n2)
Max. No. of
Electrons(2n2)
1 1 1s 1 2
2 22s2p
13
26
3 33s3p3d
135
2610
4 4
4s4p4d4f
1357
261014
![Page 11: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/11.jpg)
HOW DO THE ELECTRONS POPULATE THE AVAILABLE ORBITALS?
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Electron Spin Quantum Number, m• Two possible values are allowed
+ ½ and - ½
• Opposite directions
![Page 14: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/14.jpg)
Can two electrons in an atom have the same set of quantum numbers?
NO
![Page 15: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/15.jpg)
Pauli Exclusion Principle
• No two electrons in an atom can have the same set of four quantum numbers, n, l, ml, and ms.
• An orbital can hold a maximum of two electrons and they must have opposite spins.
![Page 16: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/16.jpg)
Electron Configuration
• The way in which electrons are distributed among the various orbitals of an atom
![Page 17: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/17.jpg)
Aufbau Principle
• Electrons occupy orbitals of lower energy first.
![Page 18: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/18.jpg)
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The relation between orbital filling and the periodic table
![Page 20: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/20.jpg)
The relation between orbital filling and the periodic table
![Page 21: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/21.jpg)
![Page 22: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/22.jpg)
Hund’s Rule
• For degenerate orbitals, the lowest energy is attained when the number of electrons with the same spin is maximized.
![Page 23: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/23.jpg)
Orbital Diagram
![Page 24: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/24.jpg)
![Page 25: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/25.jpg)
![Page 26: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/26.jpg)
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Anomalous Electron Configuration
Example:Chromium
Copper
![Page 28: Electron configuration](https://reader033.fdocuments.net/reader033/viewer/2022061116/54664c16af7959c1628b4ab1/html5/thumbnails/28.jpg)
• Consequence of the closeness of the 3d and 4s orbital energies.
• Minor departures from the expected
• Not of great chemical significance
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Seat work
Write the electron configuration and the electron orbital diagram for the following elements.
1. Cl2. Os3. Cs